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Question 5 1 pts Ethanol (C2HOH) was placed in a spirit burner and used to heat 200 cm of water in a copper can. When t...
QUESTION 3 How much heat (in kJ) is required to raise the temperature of 122 g of ethanol (mw 46.07) from 11.29 °C to i...
QUESTION 3 How much heat (in kJ) is required to raise the temperature of 122 g of ethanol (mw 46.07) from 11.29 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat - 2.46 J/g°C, AHyap = 48.6 kJ/mol) QUESTION 4 What is the change in enthalpy (in kJ) when 40.1 g of ethanol (mw-46.07) is condensed at its boiling temperature? (specific heat 2.46 J/g°C, AHvap 48.6 kJ/mol)...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol)...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be det...
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 2.99 g of FeBrz(s) are dissolved in 102.70 g of water, the temperature of the solution increases from 25.90 to 29.34 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.59 J/°C....
5) A 35.6 g sample of ethanol (C2HsOH) is burned in a bomb calorimeter, according to...
5) A 35.6 g sample of ethanol (C2HsOH) is burned in a bomb calorimeter, according to the following on. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/PC, what is the value of AHrxn? The molar mass of ethanol is 46.07 gmol C2HsOH)+302() 2 Co2()+3 H20) frxn7 A) -1.24 x 103 kJ/mol C)-809 x 103 kJ/rnol B) +1.24 x 103 kJ/mol E) +9.55 x 103 kJ/mol D) -9.55 x 103 kJ/mol...
Question 29 of 50 Submit 5.21 g of MgSO4 is placed into 100.0 mL of water....
Question 29 of 50 Submit 5.21 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate AH, in kJ/mol, for the dissolution of MgSO4 (The spe- cific heat of water is 4.18 J/g. *C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. kJ/mol 1 2 3 C +/- : 0 x 100
5) Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. When...
5) Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a temperature rise of 4.21°C was observed. The heat capacity of the bomb calorimeter excluding the water is 3.64 kJ/°C. What is the heat of combustion of naphthalene in kJ/g? (5 pts)
The salt copper(II) sulfate dissolves in water according to the reaction: CuSO4(s) ----->Cu2+(aq) + SO42-(aq) (a)...
The salt copper(II) sulfate dissolves in water according to the reaction: CuSO4(s) ----->Cu2+(aq) + SO42-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: CuSO4(s) = -771.4 kJ mol-1 Cu2+(aq) = 64.8 kJ mol-1 SO42-(aq) = -909.3 kJ mol-1 ______kJ (b) Calculate the temperature reached by the solution formed when 18.3 g of CuSO4 is dissolved in 0.195 L of water at 24.2 °C. Approximate the heat capacity of the solution by the heat capacity...
Chapter 5 and Chapter 10 Problem solving (please practice the following questions and make sure that you understand...
Chapter 5 and Chapter 10 Problem solving (please practice the following questions and make sure that you understand the principles behind: you can find Ar from textbook or website I. A 145 g sample of copper metal at 100.0°C is placed into 250.0 g of water at 25.0°C in a calorimeter. When the system reaches thermal equilibrium, the temperature of the water in the calorimeter is 28.8°C. Assume the calorimeter is perfectly insulated. What is the specific heat capacity of...
Heat Flow and Calorimetry Prelab Questions Section: Name: 1. Prepare for It! Prelab Question A A...
Heat Flow and Calorimetry Prelab Questions Section: Name: 1. Prepare for It! Prelab Question A A 235.0 g sample of metal is heated to 100.0C and poured into a calorimeter containing 50.0 g of water at 20.5°c. The equilibrium temperature of the water and metal is 30.5 C. Using the specific heat of water, 4.18 J/goC, determine the specific heat of the metal from equation 3. Use equation 5 to find the approximate molar mass of the metal. Show your...
QUESTION 3 How much heat (in kJ) is required to raise the temperature of 122 g of ethanol (mw 46.07) from 11.29 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat - 2.46 J/g°C, AHyap = 48.6 kJ/mol) QUESTION 4 What is the change in enthalpy (in kJ) when 40.1 g of ethanol (mw-46.07) is condensed at its boiling temperature? (specific heat 2.46 J/g°C, AHvap 48.6 kJ/mol)...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 2.99 g of FeBrz(s) are dissolved in 102.70 g of water, the temperature of the solution increases from 25.90 to 29.34 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.59 J/°C....
5) A 35.6 g sample of ethanol (C2HsOH) is burned in a bomb calorimeter, according to the following on. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/PC, what is the value of AHrxn? The molar mass of ethanol is 46.07 gmol C2HsOH)+302() 2 Co2()+3 H20) frxn7 A) -1.24 x 103 kJ/mol C)-809 x 103 kJ/rnol B) +1.24 x 103 kJ/mol E) +9.55 x 103 kJ/mol D) -9.55 x 103 kJ/mol...
Question 29 of 50 Submit 5.21 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate AH, in kJ/mol, for the dissolution of MgSO4 (The spe- cific heat of water is 4.18 J/g. *C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. kJ/mol 1 2 3 C +/- : 0 x 100
5) Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a temperature rise of 4.21°C was observed. The heat capacity of the bomb calorimeter excluding the water is 3.64 kJ/°C. What is the heat of combustion of naphthalene in kJ/g? (5 pts)
Chapter 5 and Chapter 10 Problem solving (please practice the following questions and make sure that you understand the principles behind: you can find Ar from textbook or website I. A 145 g sample of copper metal at 100.0°C is placed into 250.0 g of water at 25.0°C in a calorimeter. When the system reaches thermal equilibrium, the temperature of the water in the calorimeter is 28.8°C. Assume the calorimeter is perfectly insulated. What is the specific heat capacity of...
Heat Flow and Calorimetry Prelab Questions Section: Name: 1. Prepare for It! Prelab Question A A 235.0 g sample of metal is heated to 100.0C and poured into a calorimeter containing 50.0 g of water at 20.5°c. The equilibrium temperature of the water and metal is 30.5 C. Using the specific heat of water, 4.18 J/goC, determine the specific heat of the metal from equation 3. Use equation 5 to find the approximate molar mass of the metal. Show your...
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